Unit 5: chemical bonding study guide
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when elements are arranged in order of increasing atomic number; important patterns and trends emerge
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periodic law
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vertical columns
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groups
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horizontal rows
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periods
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location: left of the zig zag properties: good conductors of heat and electricity, usually solids @ room temp.
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metals
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location: right of the zig zag properties: poor conductors of heat and electricity, can be solid or liquid @ room temp
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nonmetals
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location: along zig zag properties: have both from metals and nonmetals
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semimetals
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electrons in the highest energy level -determines how an atom reacts
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valence electrons
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distance from nucleus to outermost valence electrons
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atomic radius
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the energy required to remove an electron from an atom
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ionization energy
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energy released or required when an atom gains an electron
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electron affinity
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-atoms want a full valence energy level (8 electrons) -atoms will lose, gain, or share electrons in order to achieve an octet
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octet rule
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ex. s2p4
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valence electron configuration
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link between atoms formed by electrons
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chemical bond
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energy required to break a bond
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bond energy
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formed between metal + nonmental (cation + anion) Formed by : loss or gain of electrons
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ionic bonds:
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formed between: nonmetal + nonmetal Formed by: sharing electron
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covalent bonds:
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Formed between: metal formed by: "sea" of electrons
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Metallic bonds:
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solids with high melting points brittle usually soluble in H2O good conductors when dissolved in H2O
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Properties of ionic compounds:
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a group of atoms held together by covalent bonds
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molecule
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tells number of atoms of each element in a covalent compound
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molecular formula
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electrons that are not shared (not part of a bond) in a covalent compound
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lone pairs:
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sharing 4 electrons
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double bond:
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sharing 6 electrons
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triple bond:
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Phosphorus (P) and Sulfur (S) can have 8, 10, or 12 valence electrons
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Exception of octet rule:
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1
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mono
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2
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di
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3
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tri
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4
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tetra
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5
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penta
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6
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hexa
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7
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hepta
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8
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octa
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9
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nona
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10
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dec
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Valence Shell Electron Pair Repulsion Theory -electrons will arrange themselves such that they are as far away from each other as possible
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VSEPR
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4 atoms bonded to a central atom Bond angle = 109.5
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tetrahedral
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3 atoms bonded to central atom AND 1 unshared pair on central atom bond angle = <109.5
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trigonal pyramidal
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3 atoms bonded to central atom bond angle = 120
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Trigonal Planar
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2 atoms bonded to central atom AND 2 unshared pairs on central atom Bond angle = <109.5
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Bent
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2 atoms bonded to central atom OR molecule only containing 2 atoms bond angle = 180
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Linear
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A formula showing the lowest whole number ratio of atoms in a compound
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empirical formula
